1. Gas Laws AP Physics B

2. The Periodic Table All of the elements on the periodic table are referred to in terms of their atomic mass. The symbol u is denoted as an atomic mass unit. Atomic # - # of protons OR electrons Atomic Mass - # of protons + Neutrons 1 amu = 1.66 x 10 -27 kg

3. The Mole The word “mole” is derived from Latin to mean “heap” or “pile”. It is basically a chemical counting unit. Below, what we have is called the Mole Road Map and it summarizes what a mole equals. 1 MOLE Atomic Mass from P.T Avogadro’s # = 6.02 x 10 23 Particles 22.4 Liters gas @ STP STP = Standard Temperature and Pressure ST = 0 degrees Celsius or 273 Kelvin SP = atmospheric pressure

4. Example A flexible container of Oxygen(O 2 ) has a volume of 10.0 m 3 at STP. Find the # moles and molecules that exist in the container 446.43 moles 2.68x10 26 particles

5. Factors that effect a GAS 1. The quantity of a gas, n, in moles 2. The temperature of a gas, T, in Kelvin (Celsius degrees + 273) 3. The pressure of a gas, P, in pascals 4. The volume of a gas, V, in cubic meters

6. Gas Law #1 – Boyles’ Law (complete TREE MAP) “The pressure of a gas is inverse related to the volume” Quick & Dirty:  Increasing the pressure makes balloons smaller & vice-versa as long as amount of air and temperature stay the same Moles and Temperature are constant

7. Gas Law #2 – Charles’ Law “The volume of a gas is directly related to the temperature” Quick & Dirty:  balloons get smaller when it’s cold & bigger when it’s hot as long as amount of air and pressure remain the same Pressure and Moles are constant

8. Gas Law #3 – Avogadro’s Law “The volume of a gas is directly related to the # of moles of a gas” Quick & Dirty:  balloons get bigger if you blow more air into them as long as pressure and temperature stay the same Pressure and Temperature are constant

9. Gas Law #4 – Gay-Lussac’s Law “The pressure of a gas is directly related to the temperature” Quick & Dirty:  if you put a can of spray paint above a bunsen burner, get ready to change color  doesn’t work with balloons; need a rigid container Moles and Volume are constant

10. Gas Law #5 – The Combined Gas Law You basically take Boyle’s Charles’ and Gay- Lussac’s Law and combine them together. Moles are constant

11. Example Pure helium gas is admitted into a leak proof cylinder containing a movable piston. The initial volume, pressure, and temperature of the gas are 15 L, 2.0 atm, and 300 K. If the volume is decreased to 12 L and the pressure increased to 3.5 atm, find the final temperature of the gas. 420 K

12. Gas Law #6 – The IDEAL Gas Law All factors contribute! In the previous examples, the constant, k, represented a specific factor(s) that were constant. That is NOT the case here, so we need a NEW constant. This is called, R, the universal gas constant.

13. Example A helium party balloon, assumed to be a perfect sphere, has a radius of 18.0 cm. At room temperature, (20 C), its internal pressure is 1.05 atm. Find the number of moles of helium in the balloon and the mass of helium needed to inflate the balloon to these values. 0.0244 m 3 293 K 1.05x10 5 Pa 1.052 moles